Name: ____________________________________________________
Chemistry – The Electronic Structure of the Atom Review
Properties of light
Waves
Wavelength
Frequency
Wave speed
Spectra
Electromagnetic spectrum (gammax-raysUVvisibleInfraredmicrowavesradar radio)
Visible Spectrum
(VIB G YOR)
Atomic Emission (Bright-Line) spectrum
Energy of various wavelengths above ↑ in the EM & visible spectrum
Quantum atomic model
Bohr’s model
Principle Energy Level
Ground state
Excited state
Heisenberg Uncertainty principle
Aufbau principle
Hund’s rule
Pauli’s exclusion principle
Electron Configurations
Valence electrons
Electron configurations – zip code
Orbital diagramming - arrows
Noble Gas (abbreviated) e- configs and orbital diagrams
Principal
Energy
Level
Sublevels
(Number
& Letter)
Total # of
Sublevels
Orbitals
in Sublevels
Electrons
per Sublevel
Total # of
Electrons in
Energy Level
1____________ ___________________ _________________________
_
____
2________ _2s, 2p__ ___ _2_______ 1 + 3 = 4_______ 2, 6 _____ _ 2 + 6 = 8 ___
3______________________________________________________________
_______
4______________________________________________________________
_______
5______________________________________________________________
_______
6_______________________________________________________________
______
7________________________________________________________________ ______
Answer the following questions.
____ 1. The second energy level can hold a maximum of___ electrons.
____ 2. ___ has seven electrons in its second energy level.
____ 3. The number of elements with complete 7s sublevels is ___. (use the periodic table on the wall; #106)
____4.
35Br
has ____ filled 3d orbitals.
____ 5. The first element to have the fourth energy level completely filled is ____.
____6. There are a total of____ different orbitals in the fourth energy level
____ 7. The 6 p sublevel fills with electrons after electrons enter the ____ sublevel.
____8. There are ___ orbitals filled in a theoretical filled g sublevel.
____9. The first element to have a pair of electrons in a single orbital of the 2p sublevel is___.
____10. A d sublevel can contain a maximum of _____ electron.
____11. The third energy level has ____ sublevels.
____12. The second element to have 8 electrons in a d sublevel is
____13. The only two sublevels in the valence shell are ____ and ____ sublevels.
____14. An f sublevel has ____ orbitals
____15.
79Au
has ____ electrons in its 5d sublevel
1. Einstein said light has a ‘dual nature’. What 2 things does light behave like?
2. How many electrons can a single orbital (shape) in the 3d level hold?
3. What is the principle energy level number of the 5s orbital?
4. How many different orbitals (shapes) are in the 4f sublevel?
5. Which orbital is shaped as a sphere?
6. Which orbital is shaped as a double lobe or ‘bow tie’?
7. What is the major difference between a 1s orbital and a 2s orbital, in terms of energy?
8. How many electrons are needed to fill the third principle energy level if it already contains 8 electrons?
(hint: anything with a three in front of it)
9. Electrons with the lowest possible energies are in the ___________
state.
10. How many different orbitals shapes exist in the third energy level?
11. What column of elements have 8 valence electrons? (In other words, what name do we give them?)
12. What is the full electron configuration for aluminum?
13. Which element has the following electron configuration: 1s22s22p63s23p64s1?
14. Which element has the following noble gas configuration [Kr]5s24d105p3 ?
15. Which principle states that it is impossible to know both the location and velocity (momentum) of an electron?
16. What principle states that the maximum number of electrons (with opposite spins) in each orbital shape is two e - ?
17. What rule states that electrons must “split up before they pair up” in equal energy sublevels? ↑ ↑_ ↑ before ↑↓ ↑_ ↑_
18. How many total electrons are needed to fill the second energy level?
19. How many total electrons are needed to fill 1s1 through (& including) the 4p6 orbitals?
20. Which principle energy level can only hold two electrons?
21. What is the quantum number for the energy level which can hold a maximum of 18 electrons?
22. What is the noble gas (shortcut) configuration for Bromine?
23. How many valence electrons does Tellurium have?
24. How many valence electrons does Strontium have?
25. Waves of any Electromagnetic Radiation travel at what speed?
26. When excited electrons emit light, how does their position (level jump) in the atom change?
27. Which has the longest wavelength, green light or orange light?
28. Which has the highest frequency, x-rays or infrared rays?
29. What happens to electrons when they absorb energy?
30. The number of waves to pass per second is called what?
Directions: Write out the Noble Gas configuration. (shortcut or abbreviated configuration)
1. 1s22s22p4
2. 1s22s22p63s23p64s23d104p65s24d3
3. 1s22s22p63s23p64s23d104p2
4. 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p5
Directions: Write out the longhand configuration for the following elements.
1. Si
2. Rb
3. C
Directions: Draw the orbital diagram for the following elements.
1. F
2. V
Determine the number of electrons that will be gained or lost and report whether the ion is a cation or anion. b) What noble
gas are these ions isoelectronic with?
1. Ca
2. I
Label the following electron configurations as ground state (lowest state) or excited (higher state).
Give Reasons. (remember… in an excited state an electron has moved to a higher energy level/sublevel)
1) 1s2 2s2 2p5 3p1
2) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 5d1 4f10
3) 1s2 2s2 2p6 3s2 3p6 4s2 3d5 4p5
4) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 6d1
Determine which of the following electron configurations are or are not correct, if not correct them:
1) 1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p5
2) 1s2 2s2 2p6 3s2 3d5
3) [Kr] 5s2 4d10 5p5
4) [Xe]
5) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2
Fill out the following chart.
PRINCIPAL ENERGY LEVEL
n = 1,2,3,4,5,6,7…
(Energy) SUBLEVELS (shapes)
Sublevel (letter)
Actual Shapes
_____
__________
# of individual
Orbitals in Sublevel
_____
_____
__________
_____
___________
_____
_____
__________
_____
______
Each orbital shape can hold _____ electrons.
Total # of Electrons
in each sublevel
_____
_____
_____
______